Process for recovery of minerals from acidic streams

ABSTRACT

This patent describes a method for the removal of the soluble group Ib, IIb, III, IV, V, VI, VII and VIII water soluble metallic ions from acidic streams such as acid mine drainage, pickling waste, electroplating waste wherein the waste stream contains these metal salts as pollutants which comprises: contacting said stream with a cation exchange bed containing a strong, moderately strong of weakly acidic cation exchange resin in its alkali or alkaline earth substituted form to deposit metal ions from said salts thereon, regenerating said cation exchange resin with a solution of an alkali or alkaline earth chelate and precipitating the metals by treatment with an alkali or alkaline earth base.

United States Patent Depree *May 6, 1975 [54] Eggs 2 53: 33315; M MINERALS FOREIGN PATENTS OR APPLICATIONS 1,206,038 0/1970 United Kingdom 210/28 [75] Inventor: David 0. Depree, Loomis, Calif.

OTHER PUBLICATIONS [73] Assignee: Aerojet-General Corporation, El

Monte, Calif.

Appl. No.: 323,500

Related [1.8. Application Data Continuation-impart of Ser. No. 95,252, Dec. 4, 1970, Pat. No. 3,725,259.

Stary et a1., Systematic Study of the Solvent Extraction of Metal B-Diketonates," Anal. Chim. Acta.:28( 1963). pp. 227--235.

Primary Examiner-Thomas G. Wyse Attorney, Agent, or FirmE. 0. Ansell soluble group lb, 11b, [11, IV, V, VI, VII and VIII water soluble metallic ions from acidic streams such as acid 52 us. Cl. 210/20; 210/32; 210/38 mine drainage, Pickling waste. electroplating waste 51 m 301 5 0 3021, 1 7 wherein the waste stream contains these metal salts as [58] Field of Search .1 75/101 BE; 210/24, 28, Pollutants which comprises contacting said stream 210/30, 31 R, 32, 33, 38 20 with a cation exchange bed containing a strong, moderately strong of weakly acidic cation exchange resin 5 References Cited in its alkali or alkaline earth substituted form to de- UNITED STATES PATENTS posit metal ions from said salts thereon, regenerating 2 628 165 2 l9 said cation exchange resin with a solution of an alkali 27493o6 4 22 2 33 or alkaline earth chelate and precipitating the metals 29s4276 9/1960 Haze" x by treatment with an alkali or alkaline earth base. 3,211,521 10/1965 George et a]. 75/101 BE 21 Claims, 1 Drawing Figure 3,305,306 2/1967 Morawe et al.... 210/30 X 3,388,058 6/1968 Wirth................ 210/32 3,663,163 5/1972 DePree et 210/31 X 3,725,259 4/1973 DePree............,.................... 210/30 ACID ALKAL-l O12 METAL CHELATE ALKALNJE. WASTE-[-10 EaPENT RESIN 16 5OLUT1ON I7. EARTH 1 NYC-OXIDE 1 l V V CA'I'ION QESIU EXGHMJGE ea: nsecucumou e e 2 I i i 743 1.7. |-14 5 1 aze-.3 *azwse LATE :F V 5014311014 METAL- AIEQ HYDDOXIDES PROCESS FOR RECOVERY OF MINERALS FROM ACIDIC STREAMS This application is a continuation-in-part of copending application Ser. No. 95,252, filed Dec. 4, I970, now U.S. Pat. No. 3,725,259.

BACKGROUND OF THE INVENTION It is widely recognized that modern industrial procedures have a substantial and undesirable effect on the ecology. One such source of damage to the ecology occurs in the form of waste streams from mines, pickling plants and electroplating baths. All such streams contain substantial amounts of heavy metal salts and are strongly acidic. The acidity results from hydrolyses of these salts which are salts of a weak base and strong acid. The metal salts (and acidic nature of these wastes) cause serious pollution problems if streams carrying these pollutants are discharged into streams, lakes and rivers. The present invention is believed to make a substantial contribution to the improvement of the ecology and to the specific problems associated with the disposal of certain types of industrial waste. In addition, the present invention provides a method for winning valuable metal ions from these wastes. Accordingly, it may be anticipated that the present invention will find wide application in a wide variety of industrial applications.

SUMMARY OF THE INVENTION Briefly, the present invention comprises a method for the removal of water soluble Group lb, llb, III, IV, V, VI, VII and VIII water soluble metallic ions, hereinafter referred to as heavy metal, from acidic waste streams such as acid mine drainage, pickling waste, and electroplating waste wherein the waste stream is highly acidic and contains these metal salts as pollutants which comprises: contacting said stream with a cation exchange bed containing a cation exchange resin in alkali or alkaline earth substituted form to deposit metal ions from said streams thereon, self-neutralizing the acidic effluent from the cation exchange resin, and regenerating said cation ion exchange resin with a solution of an alkali or alkaline earth chelate and precipitating the metal from said solution by treatment with an alkali or alkaline earth metal hydroxide. The alkali or alkaline earth chelate is thus recovered for recycle.

The most commonly occurring metals in acid waste streams are iron, aluminum, copper, zinc, nickel, chromium, cobalt and manganese salts, and it is the removal of these cations which is the prime objective of this invention. These can be removed when they are in any of their valence states provided that they constitute a cation, i.e., non-complexed.

It is an object of the present invention to provide a novel method for the treatment of acidic wastes.

More specifically it is an object of the present invention to provide a novel method for the removal of Groups lb, llb, III, IV, V, VI, VII and VIII water soluble metal ions from acidic waste streams. The metal ions of these groups will be called heavy metals in this specification to differentiate them from the metals of Groups Ia and Ila (alkali and alkaline earth).

It is a further object of the present invention to overcome the ecological problems associated with acid mine drainage, pickling waste, electroplating waste, and related industrial waste streams.

These and other objects and advantages of this invention will be apparent from the more detailed description which follows taken in conjunction with the accompanying drawings.

DESCRIPTION OF THE PREFERRED EMBODIMENTS The FIGURE shows a simple block diagram of the process of the present invention. The acidic waste stream is introduced through line 10 to the cation exchange bed 12. Here, the heavy metals from the stream are exchanged for the alkali or alkaline earth ions of the cation resin leaving a heavy free effluent. The product water free of heavy metals is removed by line 14 in a condition suitable for discharge into streams or further industrial non-potable uses. The spent resin from the bed 12 is passed by line 16 to the resin regeneration zone 18. The resin in the regeneration zone is treated with a solution of an alkali or alkaline earth chelate introduced by line 22. This solution exchanges alkali or alkaline earth ions for the heavy metal present in the resin prior to regeneration to form a heavy metal chelate solution which is removed via line 24 to the precipitation zone 26. The regenerated resin for zone I8 is returned to bed 12 by line 20. In the precipitation zone 26 the solution is continuously regenerated by addition of a group la or Ila metal hydroxide alone or in combination with carbon dioxide via line 28. The metal hydroxides formed within precipitation zone 26 are removed via line 30. The regenerated chelate solution thus obtained is continuously recycled by line 22 to resin regeneration zone 18. Metal ions in general have varying affinitives for particular cation exchange resins. It is possible therefore through proper resin selection and sequential displacement to favor the deposition of particular heavy metals and thus achieve selectivity in metallic ion removal. This is known in the art. In most acid waste streams a single metal predominates and hence this treatment is entirely adequate. Among the other cations found in most acid waste streams, calcium is the most common, and this is non-toxic to most mammals and therefore does not provide an environment hazard. The product water from the treatment also contains alkali and alkaline earth salts generated during the instant process. As these are non-toxic the effluent from the process does not provide an environment hazard. It may be desirable to further demineralize the effluent to complete deionization, is such is desired. Such further treatment is disclosed in U.S. Pat. No. 3,700,592 issued Oct. 24, I972 to D. O. DePree.

The present invention is applicable to both strongly and weakly acidic ion exchange resins, i.e., those within the range of complete dissociation to pH of 7.0 but is particularly applicable to the polymethacrylic cation exchange resin such as those sold under the name Am berlite CG-SO by Rohm and Haas, and others such as polyacrylic, polysalicylic acidformaldehyde polymers, phosphonic acid substituted polystyrenes, etc. Although any chelating agent which forms soluble metal chelates can be used, the preferred agents are the B- diketones (-dionates) e.g., acelylacetone, lphenylbutane-l, 3-dione, dibenzoyl methane, 2-acetylcyclohexanone and alkyl, aryl or halogen derivatives thereof. The important consideration is that the alkali or alkaline earth metal chelate and the heavy metal chelate formed be soluble in the organic solvent utilized in the It is obvious what modifications and improvements in this solubility can be achieved by modifying the B-diketone structure. The preferred solvent for the chelating agents is methanol. Other solvents which may be employed include alcohols other than methanol, e.g., ethanol, isopropanol, butanol glycols such as ethylene glycol, propylene glycol, aliphatic and aromatic ethers and polyethers, e.g., the dimethyl ethers of ethylene glycol, propylene glycol and other utilizable glycols, tetrahydrofuran and other cyclic ethers, such as dioxane.

Hydrocarbon solvents are not generally utilized alone because of solubility considerations. Other useful sol vents include DMF, DMSO, and other oxygenated solvents. Mixtures of any of the above can also be used. The chelates are usually present in an amount sufficient to form a 0. lN to 5.0N solution. The upper limit of the chelate is determined by the solubility of the metal chelate and alkali or alkaline earth chelate in the particular solvent employed. Ferric acetylacetonte, for example, is extremely soluble in methanol forming clear solution concentrations of 3 and 4 normality. The utilizeable solvents as hereby classified as regenerating solvents.

Because of the acidic nature of the water soluble salts of the heavy metals and the release of hydrogen ion during exchange cationic resins in their hydrogen form are relatively ineffective in removing these metal ions from solution. Exchange is accomplished only by partial neutralization of the stream prior to treatment. This becomes difficult when a variety of ions are present which have tendencies to form insoluble hydroxides or basic salts at different hydrogen ion concentrations. For example, iron chloride which is highly acidic in water solution due to hydrolysis may be partially neutralized to a pH of 3.0 without precipitation and this adjustment permits loading this metal ion on a polymethacrylic resin in the resin hydrogen form. Titanium tetrachloride on the other hand though also forming highly acidic water solutions due to hydrolysis is converted even at these low pH levels to the basic salt and finally the dioxide of titanium.

The need for preliminary adjustment of the acidity of the solution is eliminated in the disclosed process by the use of the cation resin in its alkali and alkaline earth form. Thus hydrogen ions since they are not present, are not liberated and the effluent is neutralized by the elution of group la or Ila ions. Thus in this process heavy metal ions displace the groups la or lla cations on the resin to give a neutral effluent as indicated in the following equations where M represents a heavy metal ion, X the anion of a strong acid, RCOO the cation resin and A an alkali or alkaline earth cation, and OH is hydroxyl ion.

RCOOA MX RCOOM AX The unique aspect of the process of this invention is that even though heavy metal salts in aqueous solution preferentially displace alkali or alkaline earth ions from cation resins, alkali and alkaline earth ions preferentially displace the heavy metal ion when the resin is treated with an alkali or alkaline earth chelate in organic solution. The following equation in which X represents a ligand (organic moiety of the chelate) illustrates this reaction.

RCOOM XA RCOOA XM The process encompasses first loading the disclosed resin efficiently with heavy metal ions from water solution, thereby providing a neutral effluent, regenerating the resin by treatment with an organic solution of an alkali or alkaline earth chelate, converting the resin to its original salt form ready for reuse. The recovered heavy metals are then precipitated from their chelate solutions by treatment of the regenerate eluate with an alkali or alkaline earth hydroxide, carbonate or basic salt, organic or inorganic, such that the alkali or alkaline earch chelate is recovered for recycle.

XM AOH M(OH) XA A neutral effluent from this demineralization process is an inherent characteristic of the process. Because the cation resin is utilized in the alkali or alkaline earth substituted form, the acidity of the feed stream is neutralized by the alkali or alkaline earth ions present on the resin. This acidity of the feedstream results from the hydrolysis of the water soluble metal salts of the Group lb, llb, lllb, lVb, Vb, Vlb, Vllb, and Vlllb metals which are present in the original feed stream. For example, a highly acidic feed stream which contains among its salts, FeSO derives its acidity from the hydrolysis of FeSO, to produce a pH of 2 to 2.5. When hydrolyzed such a salt produces a weak base and a strong acid. ln the instant process, the displacement of the alkali or alkaline earth metal ion on the resin by any of the claimed enumerated metal ions produces a salt reaction product which if hydrolyzed gives rise to both a strong acid and a strong base, i.e., a neutral salt, e.g., FeSO, Na Resin yields Fe Resin Na SO and N21 S0 is the salt of a strong acid and a strong base and is neutral in solution.

Typical bases which are employable include sodium methoxide, potassium isopropoxide, calcium bicarbonate and the lithium salt of benzyl alcohol.

The following examples are presented solely to illustrate the invention and should not be regarded as limiting in any way. In the examples the parts and percentages are by weight unless otherwise indicated.

The limitations imposed by both low pH and the liberation of hydrogen ion on the yield of deposited heavy metal ions on ion exchange resins in their hydrogen form is illustrated by the following examples of the effect of pH on the deposition of iron on a polymethacrylic acid resin.

EXAMPLE l DEPOSITION OF HEAVY METALS ON POLYMETHACRYLIC AClD RESlNS IN HYDROGEN FORM Both an acqueous solution of ferric sulfate (237 ppm} having a pH of 3.0 and a solution of ferric sulfate at a pH of 1.5 were passed sequentially through Amberlite CG-SO resin and 20 ml. fractions of eluate collected. At a pH of 1.5 no iron was deposited on the resin. At a pH of 3.0 the first two fractions were free of iron while fractions 3 and 4 showed a trace of iron to be breaking through as indicated by treatment with KCNS solution. This breakthrough occurred at about l()% of the theoretical loading capacity of the column and represents the loading which would be anticipated when H+ ions are released by FE-H-r displacement and can then act as a regenerant limiting loading of Fe-i-H-. A typical acid waste stream component ferric sulfate has a pH due to hydrolysis of 2.3.

The loading of polymethacrylic resins (weakly acidic) achieved through the displacement of a sodium ion by a heavy metal ion is illustrated in the following experiment.

EXAMPLE ll DEPOSITION OF HEAVY METAL IONS ON POLYMETHACRYLIC ACID RESINS (SODIUM LOADED) A series of 0.25 to 0.33 diameter ion exchange columns were filled with Amberlite* CG-50 resin (a polymethacrylic acid resin), 100-200 mesh particle size. Individual aqueous solutions of a variety of heavy metal salts (500 ppm concentration in metallic ion) were prepared. Each of these solutions was passed through a resin column and the eluate collected in 25 ml. fractions and analyzed for the particular metallic ion by emission spectroscopy. The metal salts selected, the Group in the Periodic Chart of the Elements represented by the metallic ion, the nature of the resin selected, the volume of solution processed prior to breakthrough, and loading achieved, is presented in the following table. A trademark of Rohm and Haas.

The following example demonstrates that alkaline earth loaded weakly acidic resins can also be used to remove heavy metal ions from aqueous solution.

5 EXAMPLE IV DEPOSITION OF CUPRIC ION ON POLYMETHACRYLIC RESIN (CALCIUM LOADED) l Copper sulfate solution (1,910 ppm in Cu-l|-), prepared by dissolving 2.4 g of CuSO in 500 ml. of deionized water, was passed through the column and 50 ml. fractions of eluate collected. Analysis of these fractions by emission spectroscopy gave the following results.

Group Volume Vol. Processed Resin Loading, Heavy Metal Salt No. Resin at Breakthrough I: of Theory Copper Sulfate lb 10 ml. 1200 30 Zinc Sulfate llb 5 ml. I150 58 Aluminum Sulfate lllb 5 ml. 150 Stannous Chloride lVb 10 ml. 25 I0 Vanadyl Sulfate Va 5 ml. 500 25 Chronium Nitrate Vla 10 ml. 600 Manganous Sulfate Vlla 5 ml. 500 Ferric Sulfate Vlll 10 ml. 250

"Eluate contained 30 ppm V and increased alter 500 ml. processed. The eluate in all instances was neutral.

EXAMPLE III REGENERATION OF HEAVY METAL LOADED RESlNS WITH A METl-IANOLIC SOLUTION OF SODIUM ACETYLACETONATE The loaded resins in the columns from Example II were each washed with 10 ml. of anhydrous methanol and then eluted with a a 1 N solution of sodium acetylacetonate in anhydrous methanol. The eluate was collected as a single sample and analyzed for heavy metal ion content by emission spectroscopy. The results obtained demonstrate the efficiency of the sodium acetylacetonate in removing the heavy metal ion by exchange.

Heavy Metal Vol. Regenerant Conc. Heavy Metal Ion Used Ion in Eluate. PPm

Cu+l- 50 I200 Zn++ 25 70 AH-H- 25 4000 Sn++ 50 I750 V+H+ 25 I250 CH-H- 50 Mn++ 25 870 Pet-H- 100 2400 Fraction No. Cone. Cu-i-h ppm The following example demonstrates that alkaline earth chelates in methanol solution readily regenerate heavy metal loaded weakly acidic resins.

EXAMPLE V REGENERATION OF CU-H' LOADED POLYMETHACRYLIC RESINS WITH CALCIUM 1,],1-TRIFLUORO-5 ,S-DIMETHY L-2,4- HEXANDIONE After washing with anhydrous methanol the loaded resin from Example IV was eluted with ml. of 0.3 N calcium I ,1 ,l -trifluoro-5 ,5-dimethyl-2,4- hexandione" prepared by dissolving 5.88 g of the dione and L1 1 g of calcium hydroxide in methanol and diluting to 100 ml.

Source Eastman organic chemical Ten ml. fractions of eluate were collected and analyzed by absorbence at 664 mu. The concentration of Cu++ in the eluate fractions were as follows:

Fraction No. Conc. Cu-H- ppm The following example demonstrates the applicability of the process to moderately acidic resin systems.

EXAMPLE VI DEPOSITION OF FERRIC ION ON POLYPHOSPHONIC ACID RESIN (SODIUM LOADED) BY ION EXCHANGE A total of 4.3 ml. of Bio Rex 63, a moderately acidic, phosphonic acid substituted resin supplied by Bio-Rad Laboratories, in its sodium salt form was charged into a 0.25 in. diameter chromatographic column. A water solution of ferric nitrate containing 3,000 ppm of Fe+-+lwas prepared and passed through the column and 50 ml. fractions of eluate collected and analyzed for ferric ion by light absorption at 440 um.

Fraction No. Conc. Fe-l-H, ppm

l l 2 l 3 360 4 550 The following example demonstrates that heavy metal ions are readily removed from moderately acidic ion exchange resins with alkali metal chelate solutions.

EXAMPLE VII REGENERATION OF Fe-l-l-i- LOADED POLYPHOSPHONIC ACID RESIN WITH SODIUM ACETYL ACETONATE After washing with anhydrous methanol the loaded resin from Example VI was eluated with a l N solution of sodium acetylacetonate in methanol (total of 25 ml) and 5 ml. fractions of eluate collected and analyzed by the same procedure described in Example VI. The analytical data obtained were as follows:

Fraction No. Conc. Fe-l+-+, ppm

un-t wru- The following example shows that even strongly acidic resins may be used in this process.

EXAMPLE VIII DEPOSITION OF MANGANOUS ION ON POLYSULFONIC ACID RESIN (SODIUM LOADED) BY ION EXCHANGE A volume of 9.5 ml. of sodium loaded AG-SOW-X8 resin, a strongly acidic, styrene based. polysulfonic acid resin manufactured by Dow Chemical Company was charged into a 0.33 in. diameter chromatographic column. An aqueous solution of manganous sulfate having a concentration of 6,500 ppm ion was passed through the column and 50 ml. fractions of eluate collected and analyzed for manganese ion by emission spectroscopy. The results of these analyses were as follows:

Fraction No. Conc. Mn++, ppm

The following example illustrates the removal of heavy metals from strongly acidic resins with an alkali metal chelate solution.

EXAMPLE IX REGENERATION OF Mn-H- LOADED POLYSULFONIC ACID RESIN WITH SOIDUM ACETYL ACETONATE After washing with anhydrous methanol the resin from Example VIII was eluted with ml. of a 0.25 N solution of sodium acetonate in methanol containing l% by volume of deionized water. Twenty-five ml. fractions of eluate were collected and analyzed for Mn++ concentration by UV absorbance. The analytical results were as follows:

Fraction No. Conc. Mn-H- The following examples X and XI illustrate the fact that mixtures of heavy metals may be deposited on the resin and removed by subsequent regeneration.

EXAMPLE X DEPOSITION OF A MIXTURE OF HEAVY METAL IONS ON POLYMETHACRYLIC ACID RESIN (SODIUM FORM) BY ION EXCHANGE A 10 ml. volume of sodium loaded Amberlite CG-SO resin, a weakly acidic, polymethacrylic acid resin manufactured by Rohm and Haas Co., was

charged to a 0.4 in diameter chromatographic column. A trademark of Rohm and Haas.

Concentration, ppm

Fa l-H Cu++ Co-l-t- EXAMPLE XI REGENERATION OF Fe-lil-, Co-l-iand Cu++ LOADED POLYMETHACRYLIC ACID RESIN WITH SODIUM ACETYL ACETONATE The loaded resin from Example X was washed with 50 ml. of anhydrous methanol. The resin was then eluted with 50 ml. of a lN. solution of sodium acetylacetonate ir anhydrous methanol. A total of two 25 ml. fractions of eluate were collected. These fractions were analyzed by emission spectroscopy and the following results obtained.

Concentration, ppm Fraction No. Feh-H- CcH-l- Cu++ The fractions are combined, and a slight excess of sodium hydroxide in methanol solution is added with stirring to the eluate with resultant precipitation of the heavy metal hydroxides.

The precipitate is now ready for selective separation as desired by utilizing the differences in the amphoteric properties of the various metals.

As shown previously, in Example IX, anhydrous organic solvents are not required. Up to about l% of deionized water may be added to the utilized solvent, provided that the eluted heavy metal chelate is soluble in the mixed solvent system and further provided that the organic solvent is fully mixable with water. In some instances small additions of water to the elute is desirable to maintain the resin in its swollen form to ensure efficient diffusion of the regenerant solution into the resin.

The process of the instant invention can be carried out independent of temperature and pressure.

Since the process here is an ion displacement process, rather than a demineralization process, it is seen that the acid strength of the resin is not a critical parameter. Hence any cationic resin which forms metallic salts can be employed.

The concentrations of heavy metal ions present in the original aqueous solution to be environmentally purified has no bearing on the ability of the process to operate. Plant size considerations (bed size, column diameter, and the like) are the only practical limitations on the practice of this invention.

The process, as demonstrated in the preceding examples, has been shown in most instances, even at high concentration of heavy metal ion to give essentially complete environmental purification (heavy metal ion removal).

The concentration of the regenerant solution is limited only by the solubility of the Group la and/or Group Ila chelate employed.

It is also to be seen that a mixture of at least one Group Ia and at least one Group Ila metal chelates can be used in combination.

It is further to be seen that in some instances it may be desirable to employ mixtures of resins each of which has a different acid strength to achieve higher resin loadings.

It is obvious that while the disclosure has demonstrated the removal of certain heavy metal ions on particular resins, equally satisfactory results are obtainable when other metal ions of the set forth groups are treated with other cationic resins in the alkalie earth or alkali metal form.

A skilled chemist being cognizant of the oxidative capacity of certain heavy meatal ions may find it desirable to conduct the process in the absence of oxygen.

It is seen that the instant process is utilizeable only with those heavy metals which form cations in aqueous solution. Thus titanium tetrachloride, which is often present in industrial waste and which is not stable in aqueous media but forms the dioxide by hydrolysis, even at pl-Is as low as about I, is therefore incapable of having the titanium ion removeable. The process is utilizeable for all heavy metals as prevously defined and in particular with respect to the transition metals.

Other heavy metal ions such as chromium can appear both as the cgtion, Cr+++, in anionic form, the chromate CrO-4 and thus only the former ionic form is removeable by the insant process.

Although the process would customarily be carried out by passing the aqueous solution of the heavy metals through a fixed ion exchange bed, other state of the art techniques such as back flow processes, countercurrent processes, or slurry techniques may be employed.

Although the process has primary application to streams that constitute an environmental hazard such as acid mine waste (iron, monganese, aluminum and perhaps copper from coal and other mineral mining processes), electroplating wastes (chromium, tin, copper, zinc and nickel plating techniques) and pickling wastes (iron and vanadium passivation and surface cleaning operations, the instant process is applicable to metal winning from natural streams such as sea water, certain mountain runoff streams and may even find application in a metal refining process where an acid leach is initially employed to extract metals from raw ores. This application is described in the following example.

EXAMPLE XII EXTRACTION AND RECOVERY OF HEAVY METAL IONS FROM ORE Four grams of Bornite, which contains the metals copper and iron and has the chemical structure of Cu FeS was heated in a concentrated solution of HCl 4 for 24 hours to leach out at least part of the heavy metal in content. The green colored solution was filtered to remove suspended materials diluted to 1,000 ml. and analyzed by emission spectroscopy for metal ion content which was determined to be as follows:

Concentration of Heavy Metals, ppm

Cu i-i- Fe+++ Back weighing the suspended materials removed by the above filtration yielded 3.4 grams of materials other than Cu, Fe and S.

These metal sulfates are now in a form suitable for removal by the instant process. Removal of these ions by the instant process was accomplished by passing the green colored sulfate solution after adjusting the pH to 2.5 to neutralize excess HCl through a 0.4 in. diameter column which contained mil. of Amberlite* CG50 resin (polymethacylic acid in its sodium substituted form). while still warm (about 35C). Several ml. fractions were collected of the eluate, and analyzed for heavy metal ion content. The results are as follows:

EXAMPLE XIII EXTRACTION OF HEAVY METAL FROM ORE AND DEPOSITION ON CATION EXCHANGE RESIN Six and one-half grams of Rhodocrosite, an ore which contains the metal manganese in the chemical form of manganese carbonate, was leached with ID ml. of con centrated hydrochloric acid over a 16 hr. period. Essentially all of the ore disolved with the evolution of carbon dioxide. The light pink solution (manganous chloride) was filtered to remove a trace of suspended material and diluted to 1,000 ml. with dionized water. The pH of the diluted solution was found to be approximately 5 indicating that no excess mineral acid remained. The manganese content of the diluted solution was determined to be approximately 3,000 ppm.

The above solution was then contacted with l0 ml. of Amberlite* CG-SO resin (a weakly acidic, polymethacrylic resin in its sodium form) using a 0.5 in. diameter chromatographic column. The resin developed a yellow tan color on deposition of manganese. A total of 290 ml. of eluate from the column was collected before breakthrough of manganese occured.

These examples show that heavy metals can be removed from their ores and their ions separated by adaption of the instant process. The ore processing product water discharged and/or collected is free of heavy metal cationic pollutants. This water can either be discharged directly into the environment or after further treatment to remove Group la and Group Ila salts at the option of the processor as may be required by appropriate regulation. This ore processing product water, after the Group la and lla salt concentration is lowered to acceptable levels, depending upon intended application, may be utilized for agriculture, potable water and industrial purposes. I

As previously mentioned, any chelating agent known to the art which provides an organic solvent system soluble alkali (La, K, Li, Cs, Rb) Group la or alkaline earth (Ca, Mg, Ba, Be, Sr) Group Ila chelate is employ able herein provided that the heavy metal ion(s) to be removed also is/are soluble in the same solvent system. Thus other chelates besides the preferred B-dionates, such as aryl or alkyl substituted phosphates, e.g., phenyl phosphate, and di-n-octyl phosphate, alkyl or aryl substituted phosphites, e.g., di'2-ethylhexyl phosphite and diphenyl phosphite, esters of B-dicarcoxylates, e.g., diethyl malonate.

It is to be understood that either or both of the steps of initially contacting the resin with the solution of heavy metal ions, and also the regeneration step can be carried out using fixed resin beds, fluidized concurrent beds, and fluidized counter-current beds and any combination thereof with equally satisfactory results. The mode of carrying out each of the two steps is dependent upon economic, and engineering considerations taking into account the metals to be removed.

While I have demonstrated by examples the deposi tion of specific metals on certain resins, similar results are obtainable for all of the water soluble heavy metal cations when deposited on any of the resin types disclosed, i.e., weakly acidic, moderately acidic or strongly acidic resins.

Although the invention has been described in considerable detail in the foregoing for the purpose of illustration, it is to be understood that such detail is solely for this purpose and that variations can be made by those skilled in the art without departing from the spirit and scope of the invention except as is set forth in the claims.

What I claim is:

l. A method for the removal of water soluble Group lb, llb, Vb, VIb, Vllb, and Vlllb metallic ions from highly acidic water solutions containing said ions which comprises initially contacting the solution with a cation exchange resin, which resin is present as the alkali or alkaline earth form thereof, depositing the water solu ble metallic ions on said resin, providing a neutral effluent, and regenerating the cation exchange resin by contacting same with a regenerating solvent solution of an alkali or alkaline earth chelate.

2. The process of claim 1 including the additional step of precipitating said metallic ions from the regenerating solvent solution by the addition of an alkali or alkaline earth base.

3. The process of claim 2 wherein at least two metallic ions are removed by contact with the cation exchange resin.

4. The process of claim 3 wherein the chelate employed is a B-dionate.

5. The process of claim 4 wherein the solvent employed is a compound having at least one hydroxyl group.

6. The process of claim 2 wherein the initial contact and the regeneration steps are carried out in one of the following types of cation exchange beds, fixed, fluidized concurrent, and fluidized countercurrent, a different bed mode being utilized for each step.

7. The method of claim 1 wherein the regeneration step is carried out in an alcoholic solution of the chelate.

8. The method of claim 7 wherein the alcoholic solution contains methanol.

9. The method of claim 1 wherein the chelate is a betadionate.

10. The method of claim 9 wherein the betadionate is selected from the group consisting of acetylacetone and Z-acetylcyclohexanone.

11. The process of claim 1 wherein the chelate is selected from the group consisting of organic phosphates, organic phosphites and esters of B-dicarboxylates.

12. The process of claim 1 wherein the contacting consists of passing the solution of the metallic ions through a cation exchange bed which is a fixed bed.

13. The process of claim 12 wherein the cation exchange bed is a fluidized bed.

14. The process of claim 13 wherein the contacting and regeneration steps are carried out in a countercurrent fashion.

15. The process of claim 1 wherein both the initial contacting and the regeneration steps are carried out in a fixed bed.

16. The process of claim 1 wherein both the initial contacting and the regeneration steps are carried out in a fluidized bed.

17. The process of claim 16 wherein the contacting and regeneration steps are carried out in a countercurrent fashion.

18. The process of claim 1 wherein at least two metallic ions are removed by contact with the cation exchange resin.

19. A process for the removal of transition metal ions from highly acidic water solutions containing said ions which comprises contacting the solution with a polymethacrylic acid type ion exchange resin in its alkali metal or alkaline earth metal substituted form, depositing the transition metals thereupon and simultaneously providing a neutral effluent from the exchange including the additional step of regenerating the cation exchange resin in a regeneration solvent solution with a chelate.

20. The process of claim 19 which comprises the additional steps of precipitating said transition metal ions by the addition of an alkali or alkaline earth base to the solvent solution from the regeneration step.

21. The process of claim 20 which comprises carrying out the regeneration step with alcoholic solution of a chelate selected from the group consisting of alkali and alkaline earth betadionates.

* III I t 

1. A METHOD FOR THE REMOVAL OF WATER SOLUBLE GROUP 1B, 11B, VB, V1B, V11B, V111B METALLIC IONS FROM HIGHLY ACIDIC WATER SOLUTIONS CONTAINING SAID IONS WHICH COMPRISES INITALLY CONTACTING THE SOLUTION WITH A CATION EXCHANGE RESIN, WHICH RESIN IS PRESENT AS THE ALKALI OR ALKALINE EARTH FROM THEREOF, DEPOSITING THE WATER SOLUBLE METALLIC IONS ON SAID RESIN, PROVIDING A NEUTRAL EFFLUENT, AND REGENERATING THE CATION EXCHANGE RESIN BY CONTACTING SAME WITH A REGENERATING SOLVENT SOLUTION OF AN ALKALI OR ALKALINE EARTH CHELATE.
 2. The process of claim 1 including the additional step of precipitating said metallic ions from the regenerating solvent solution by the addition of an alkali or alkaline earth base.
 3. The process of claim 2 wherein at least two metallic ions are removed by contact with the cation exchange resin.
 4. The process of claim 3 wherein the chelate employed is a B-dionate.
 5. The process of claim 4 wherein the solvent employed is a compound having at least one hydroxyl group.
 6. The process of claim 2 wherein the initial contact and the regeneration steps are carried out in one of the following types of cation exchange beds, fixed, fluidized concurrent, and fluidized countercurrent, a different bed mode being utilized for each step.
 7. The method claim 1 wherein the regeneration step is carried out in an alcoholic solution of the chelate.
 8. The method of claim 7 wherein the alcoholic solution contains methanol.
 9. The method of claim 1 wherein the chelate is a betadionate.
 10. The method of claim 9 wherein the betadionate is selected from the group consisting of acetylacetone and 2-acetylcyclohexanone.
 11. The process of claim 1 wherein the chelate is selected from the group consisting of organic phosphates, organic phosphites and esters of B-dicarboxylates.
 12. The process of claim 1 wherein the contacting consists of passing the solution of the metallic ions through a cation exchange bed which is a fixed bed.
 13. The process of claim 12 wherein the cation exchange bed is a fluidized bed.
 14. The process of claim 13 wherein the contacting and regeneration steps are carried out in a counter-current fashion.
 15. The process of claim 1 wherein both the initial contacting and the regeneration steps are carried out in a fixed bed.
 16. The process of claim 1 wherein both the initial contacting and the regeneration steps are carried out in a fluidized bed.
 17. The process of claim 16 wherein the contacting and regeneration steps are carried out in a counter-current fashion.
 18. The process of claim 1 wherein at least two metallic ions are removed by contact with the cation exchange resin.
 19. A process for the removal of transition metal ions from highly acidic water solutions containing said ions which comprises contacting the solution with a polymethacrylic acid type ion exchange resin in its alkali metal or alkaline earth metal substituted form, depositing the transition metals thereupon and simultaneously providing a neutral effluent from the exchange including the additional step of regenerating the cation exchange resin in a regeneration solvent solution with a chelate.
 20. The process of claim 19 which comprises the additional steps of precipitating said transition metal ions by the addition of an alkali or alkaline earth base to the solvent solution from the regeneration step.
 21. The process of claim 20 which comprises carrying out the regeneration step with alcoholic solution of a chelate selected from the group consisting of alkali and alkaline earth betadionates. 